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Consider the following electrochemical cell: Pt | H₂(g,pᵒ) | HCl(aq,b) | Hg₂Cl₂(s) | Hg(1) The potential of this cell, in relation to different molalities (b), has been measured with high precision at 25°C. The following results have been obtained: b/mmol.kg¹ E/V I (ionic strength) Y+ (DHLL) Y+ (linear fit) (ii) (iii) (iv) 1.6077 0.60080 3.0769 0.56825 (x) 5.0403 0.54366 7.6938 0.52267 (i) Write the half-reactions for the cell, and show the standard potential of each half-reaction. Determine the standard cell potential through simple calculation. Write the cell reaction for this cell. 10.9474 0.50532 Write the Nernst equation for this cell in terms of molality (b) and the mean activity coefficient (y+) of HCI. (v) Determine the ionic strength (I) for each molality (b) (and complete the above table). (vi) By employing the Debye-Hückel limiting law (DHLL), determine the mean activity coefficient (y) of HCI (and complete the above table). (vii) Write the Nernst equation for this cell only in terms of molality (b), where the mean activity coefficient (Y) of HCI does not feature. (viii) Rearrange the equation in (vii) and make a suitable plot, using the data in the table, to determine the standard cell potential. (ix) Now incorporate the standard cell potential, determined from the linear fit in (viii), into the Nernst equation and determine the mean activity coefficient (y) of HCI (and complete the above table). Comment on any differences that you might observe between the values obtained for the mean activity coefficient (y) of HCI in (vi) and (ix). Show all your calculations and derivations, however, for (v), (vi) and (ix) you only have to show one set for each of the calculations.

Consider the following electrochemical cell: Pt | H₂(g,pᵒ) | HCl(aq,b) | Hg₂Cl₂(s) | Hg(1) The potential of this cell, in relation to different molalities (b), has been measured with high precision at 25°C. The following results have been obtained: b/mmol.kg¹ E/V I (ionic strength) Y+ (DHLL) Y+ (linear fit) (ii) (iii) (iv) 1.6077 0.60080 3.0769 0.56825 (x) 5.0403 0.54366 7.6938 0.52267 (i) Write the half-reactions for the cell, and show the standard potential of each half-reaction. Determine the standard cell potential through simple calculation. Write the cell reaction for this cell. 10.9474 0.50532 Write the Nernst equation for this cell in terms of molality (b) and the mean activity coefficient (y+) of HCI. (v) Determine the ionic strength (I) for each molality (b) (and complete the above table). (vi) By employing the Debye-Hückel limiting law (DHLL), determine the mean activity coefficient (y) of HCI (and complete the above table). (vii) Write the Nernst equation for this cell only in terms of molality (b), where the mean activity coefficient (Y) of HCI does not feature. (viii) Rearrange the equation in (vii) and make a suitable plot, using the data in the table, to determine the standard cell potential. (ix) Now incorporate the standard cell potential, determined from the linear fit in (viii), into the Nernst equation and determine the mean activity coefficient (y) of HCI (and complete the above table). Comment on any differences that you might observe between the values obtained for the mean activity coefficient (y) of HCI in (vi) and (ix). Show all your calculations and derivations, however, for (v), (vi) and (ix) you only have to show one set for each of the calculations.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 76AP
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Consider the following electrochemical cell: Pt | H₂(g,pᵒ) | HCl(aq,b) | Hg₂Cl₂(s) | Hg(1) The potential of this cell, in relation to different molalities (b), has been measured with high precision at 25°C. The following results have been obtained: b/mmol.kg¹ E/V I (ionic strength) Y+ (DHLL) Y+ (linear fit) 1.6077 0.60080 (ii) (iii) (iv) 3.0769 0.56825 5.0403 0.54366 7.6938 0.52267 10.9474 0.50532 (i) Write the half-reactions for the cell, and show the standard potential of each half-reaction. Determine the standard cell potential through simple calculation. Write the cell reaction for this cell. Write the Nernst equation for this cell in terms of molality (b) and the mean activity coefficient (y) of HCI. (v) (vi) (vii) Write the Nernst equation for this cell only in terms of molality (b), where the mean activity coefficient (Y) of HCI does not feature. (viii) Rearrange the equation in (vii) and make a suitable plot, using the data in the table, to determine the standard cell potential. (ix) Now incorporate the standard cell potential, determined from the linear fit in (viii), into the Nernst equation and determine the mean activity coefficient (y) of HCI (and complete the above table). (x) Comment on any differences that you might observe between the values obtained for the mean activity coefficient (y) of HCI in (vi) and (ix). Determine the ionic strength (I) for each molality (b) (and complete the above table). By employing the Debye-Hückel limiting law (DHLL), determine the mean activity coefficient (y) of HCI (and complete the above table). Show all your calculations and derivations, however, for (v), (vi) and (ix) you only have to show one set for each of the calculations.
Transcribed Image Text:Consider the following electrochemical cell: Pt | H₂(g,pᵒ) | HCl(aq,b) | Hg₂Cl₂(s) | Hg(1) The potential of this cell, in relation to different molalities (b), has been measured with high precision at 25°C. The following results have been obtained: b/mmol.kg¹ E/V I (ionic strength) Y+ (DHLL) Y+ (linear fit) 1.6077 0.60080 (ii) (iii) (iv) 3.0769 0.56825 5.0403 0.54366 7.6938 0.52267 10.9474 0.50532 (i) Write the half-reactions for the cell, and show the standard potential of each half-reaction. Determine the standard cell potential through simple calculation. Write the cell reaction for this cell. Write the Nernst equation for this cell in terms of molality (b) and the mean activity coefficient (y) of HCI. (v) (vi) (vii) Write the Nernst equation for this cell only in terms of molality (b), where the mean activity coefficient (Y) of HCI does not feature. (viii) Rearrange the equation in (vii) and make a suitable plot, using the data in the table, to determine the standard cell potential. (ix) Now incorporate the standard cell potential, determined from the linear fit in (viii), into the Nernst equation and determine the mean activity coefficient (y) of HCI (and complete the above table). (x) Comment on any differences that you might observe between the values obtained for the mean activity coefficient (y) of HCI in (vi) and (ix). Determine the ionic strength (I) for each molality (b) (and complete the above table). By employing the Debye-Hückel limiting law (DHLL), determine the mean activity coefficient (y) of HCI (and complete the above table). Show all your calculations and derivations, however, for (v), (vi) and (ix) you only have to show one set for each of the calculations.
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